# Problem: At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.44 x 103.2NO (g) ⇌ N2 (g) + O2 (g)A closed vessel is charged with 26.1 atm of NO. What is the partial pressure of N2 at equilibrium?a. 0.726 atmb. 3.21 atmc. 12.92 atmd. 2.88 atme. 18.16 atm

###### FREE Expert Solution

We’re being asked to determine the equilibrium pressure of N2 given the following equilibrium reaction:

2NO (g) ⇌ N2 (g) + O2 (g)

When dealing with equilibrium and Kc:

Kp → equilibrium units are in atm
Kp is an equilibrium expression:

$\overline{){\mathbf{Kp}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the pressure in the equilibrium expression

Given:

Initial pressure:

NO = 26.1 atm

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###### Problem Details

At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.44 x 103.

2NO (g) ⇌ N2 (g) + O2 (g)

A closed vessel is charged with 26.1 atm of NO. What is the partial pressure of N2 at equilibrium?

a. 0.726 atm

b. 3.21 atm

c. 12.92 atm

d. 2.88 atm

e. 18.16 atm